IMG_0001_NEW_0032

IMG_0001_NEW_0032 - *owt to+;,'^'[hy a -fua 2- cE'N) 7o - {...

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Let's look at point c) (above) in a little more detail The fluoride anion (F-) is much smaller than iodide (I ) and has a much larger chargelsize ratio. In solution, the fluoride anion will be solvated to a greater extent than iodide. This solvation blocks it from sharing electrons (or reacting) with an electrophile. We rnust also consider poTarizability or ease n'ith ri'hich eiectrons can be delocalized over the surface of an atom. Fo'e-a,,a halil 40lr"U *n C-,=tU!-
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Unformatted text preview: *owt to+;,'^'[hy a -fua 2- cE'N) 7o - { e lrln kzs 4/4 -,. lrty W -t" egpe- ,>t ndff Consider the followins ecuations: o -,P -P $o-:Hd.-dx NA fu<o IF () e.g. H,-I tu?dd'i pLa t c.A -r ?U is la4e-" M"4' ta/qd'-b What about electrophiles? The more positively charged the atom, the better able it is to accept an electron pair from a nucleophile and form a new bond. {p \e2 ^Jo dowk@ HJ [-"=H ili ' llvL oqll e@wor*;(e-Y 6il \r' dr*arrof$Ml-a CP-bvA E"...
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